Dinitrogen pentoxide is an ionic compound formed from the ions NO2^+ and NO3^-. Give the oxidati

Name: Problem 56, Chapter 24: Chemistry A Molecular Approach
Uploaded: 2020-03-21T19:51:23-08:00
Duration: 3 min 55 s
Channel: Ahmed Ali
Description: Dinitrogen pentoxide is an ionic compound formed from the ions NO2^+ and NO3^-. Give the oxidation state of N in each ion and the VSEPR shape for each of the ions.

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Question

Dinitrogen pentoxide is an ionic compound formed from the ions $\mathrm{NO}_{2}^{+}$ and $\mathrm{NO}_{3}^{-}$. Give the oxidation state of $\mathrm{N}$ in each ion and the VSEPR shape for each of the ions.

   Dinitrogen pentoxide is an ionic compound formed from the ions $\mathrm{NO}_{2}^{+}$ and $\mathrm{NO}_{3}^{-}$. Give the oxidation state of $\mathrm{N}$ in each ion and the VSEPR shape for each of the ions.

Chemistry A Molecular Approach

Nivaldo J. Tro 5th Edition

Chapter 24, Problem 56

Instant Answer

Solved by Expert Ahmed Ali

03/21/2020

Step 1

Determine the oxidation state of N in each ion: In NO2+ ion: - Oxygen has an oxidation state of -2. - There are two oxygen atoms, so the total oxidation state of oxygen in the ion is -4. - The ion has a charge of +1, so the oxidation state of N in NO2+ must be +3 Show more…

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Dinitrogen pentoxide is an ionic compound formed from the ions $\mathrm{NO}_{2}^{+}$ and $\mathrm{NO}_{3}^{-}$. Give the oxidation state of $\mathrm{N}$ in each ion and the VSEPR shape for each of the ions.

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Key Concepts

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) theory is used to predict the three-dimensional geometry of molecules and polyatomic ions based on the repulsion between electron pairs (bonding and lone pairs) around a central atom. By determining the number of electron groups, one can infer molecular shapes, such as linear or trigonal planar, which are important for understanding chemical behavior and molecular interactions.

Oxidation State Determination

This concept involves assigning oxidation numbers to atoms in a compound or ion using systematic rules, such as assuming a typical oxidation state for oxygen and using the overall charge of the ion to calculate the unknown oxidation states. It is fundamental in understanding electron distribution, predicting reactivity, and balancing redox reactions.

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